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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Relationship of Kc and Kp:

  1. (a) Kp for the following reaction is 0.16 at 25 °C. What is the value of Kc?

    2 NOBr(g) ⇄ 2 NO(g) + Br2(g)

  2. (b) The equilibrium constant, Kc, for the following reaction is 1.05 at 350 K. What is the value of Kp?

    2 CH2Cl2(g) ⇄ CH4(g) + CCl4(g)

(a)

Interpretation Introduction

Interpretation: The value of Kc for the given reaction has to be calculated

Concept introduction:

  • Equilibrium constant: It is the ratio of products to reactants has a constant value when the reaction is in equilibrium at a certain temperature. And it is represented by the letter K.

  For a reaction,

  aA+bBcC+dD

  The equilibrium constant is, K=[C]c[D]d[A]a[B]b, where, a, b, c and d are the stoichiometric coefficients of reactant and product in the reactions.

  • Kc is the equilibrium constant of a reaction at equilibrium which is expressed in terms of concentration of gaseous reactants and products. Whereas Kp is the equilibrium constant of a reaction at equilibrium which is expressed in terms of partial pressure of gaseous reactants and products in a closed system.

  Kp=Kc(RT)Δn where,Δn is difference between the sum of stoichiometric coefficients of products and reactants.

Explanation

Kc for the given equation is calculated as,

Given,

  R=0.08206L.atm K1mol1T=250C=(25+273)K=298KKp=0.16

The balanced chemical equation for the reaction is,

  2NOBr(g)2NO(g)+Br2(g)

Hence,

  Δn=32

(b)

Interpretation Introduction

Interpretation: The value of Kp for the given reaction has to be calculated.

Concept introduction:

  • Equilibrium constant: It is the ratio of products to reactants has a constant value when the reaction is in equilibrium at a certain temperature. And it is represented by the letter K.

  For a reaction,

  aA+bBcC+dD

  The equilibrium constant is, K=[C]c[D]d[A]a[B]b, where, a, b, c and d are the stoichiometric coefficients of reactant and product in the reactions.

  • Kc is the equilibrium constant of a reaction at equilibrium which is expressed in terms of concentration of gaseous reactants and products. Whereas Kp is the equilibrium constant of a reaction at equilibrium which is expressed in terms of partial pressure of gaseous reactants and products in a closed system.

  Kp=Kc(RT)Δn where,Δn is difference between the sum of stoichiometric coefficients of products and reactants.

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